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{"ops":[{"insert":"C = (\u00b0F \u2013 32) *5\/9                                              \u00b0F = \u00b0C * 9\/5 + 32                                             K = \u00b0C + 273\r\n      G =    H - T     S (Gibbs Formula)\r\n   Where: Delta H is change in Enthalpy, T is temperature (in Kelvin), and Delta S is change in entropy\r\n\r\n1. Calculate the Gibbs free energy change (  G ) for the following chemical reaction:  \r\n ATP                          ADP + Pi \r\n The reaction occurs at 65 \u00b0F, the change in heat (H) = 18,180 cal, and the change in entropy (S) = 86 cal\/K.\r\n\r\n2. Calculate the Gibbs free energy change (G) for the following chemical reaction:  \r\n glutamate + NH3                       glutamine + H2O \r\n The reaction occurs at 68 \u00b0F, the change in heat (H) = 4113 cal, and the change in entropy (S) = 2.6 cal\/K.\r\n\r\n3. Would either of the reactions above occur spontaneously?  If so, which one(s) and why?\r\n\r\n4. How does the Gibbs free energy in each of the two reactions change if the temperature were raised to normal body temperature (92.8 \u00b0F)?\r\n\r\n5. Does an increase in reaction temperature make each of these reactions more or less likely to occur spontaneously?  Explain your answer.\r\n\n"}]}

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